if H and S are both negative
A high temperature will make it spontaneous.
For some non-spontaneous reactions, you can change the temperature. For other non-spontaneous reactions, there is nothing you can do to make it spontaneous. Nature favors reactions that increase a system's entropy (disorder) and nature favors reactions that are exothermic (they release enthalpy). Any reaction that does both of these things is spontaneous at all temperatures. Any reaction that does neither of these things is never spontaneous. As far as this question is concerned, the interesting reactions are endothermic reactions that increase entropy and exothermic reactions that decrease entropy. Whether these reactions are spontaneous depends on the temperature. The first variety (endothermic, increase entropy) will be spontaneous at high temperatures; the second (exothermic, decrease entropy) will be spontaneous at low temperatures. To find the temperature at which a reaction becomes spontaneous, one may apply the Gibbs equation: DG = DH - TDS where capital Ds stand for the Greek capital delta.
∆G = ∆H - T∆S and for it to be spontaneous, ∆G should be negative. If both ∆H and ∆S are positive, in order to get a negative ∆H, the temperature needs to be elevated in order to make the ∆S term greater than the ∆H term. So, I guess the answer would be "the higher the temperature, the more likely will be the spontaneity of the reaction."
Optimum temperature and pH medium make suitable conditions for enzymatic reactions.
no the reaction is not bigger, but it does last longer with cold vinegar.
if H and S are both negative
A high temperature will make it spontaneous.
A high temperature will make it spontaneous.
When H and S are both positive
For some non-spontaneous reactions, you can change the temperature. For other non-spontaneous reactions, there is nothing you can do to make it spontaneous. Nature favors reactions that increase a system's entropy (disorder) and nature favors reactions that are exothermic (they release enthalpy). Any reaction that does both of these things is spontaneous at all temperatures. Any reaction that does neither of these things is never spontaneous. As far as this question is concerned, the interesting reactions are endothermic reactions that increase entropy and exothermic reactions that decrease entropy. Whether these reactions are spontaneous depends on the temperature. The first variety (endothermic, increase entropy) will be spontaneous at high temperatures; the second (exothermic, decrease entropy) will be spontaneous at low temperatures. To find the temperature at which a reaction becomes spontaneous, one may apply the Gibbs equation: DG = DH - TDS where capital Ds stand for the Greek capital delta.
Spontaneous ...Happens all by itself; typically unpredictableNon-spontaneous...You have to do something to make it happen.
when h and s are both positive
There was a spontaneous reaction of elation when the local lottery syndicate won one million pounds.
Reactions are described by this equation: GD = HD - TDS where D = delta for change in values. GD < 0 spontaneous HD < 0 exothermic ; HD > 0 endothermic The first equation is Gibbs free energy. When G is negative, the reaction is spontaneous. In contrast, a positive number G is non spontaneous. The interesting thing is that spontaneous reactions can be EITHER exothermic and endothermic. Lets look at this: lets assume HD has a value of 100. This means TDS would have to be bigger than 100 in order to make GD a negative number. An endothermic reaction which has a positive H can still be exothermic. Here's another way to pose your question: Is an exothermic reaction spontaneous? Always. Is an endothermic reaction spontaneous? This can be either.
∆G = ∆H - T∆S and for it to be spontaneous, ∆G should be negative. If both ∆H and ∆S are positive, in order to get a negative ∆H, the temperature needs to be elevated in order to make the ∆S term greater than the ∆H term. So, I guess the answer would be "the higher the temperature, the more likely will be the spontaneity of the reaction."
No. A spontaneous reaction is one that will happen given enough time - it doesn't need any energy or enzyme to make it happen. For instance, the decomposition of carbonic acid (H2CO3) into water and carbon dioxide (H2O and CO2) is spontaneous. However, it can be reversed by an enzyme called carbonic anhydrase; it just takes energy.
You can actually control production of products or consumption of reactants by changing the physical conditions like temperature and pressure. In industrial manufacturing of Ammonia, it is desirable to get as much product (ammonia) as possible, hence manufacturers continue the reaction to do so.